Question

how are bond angles of molecules affected by electronegativity explain taking example of NH3 ,NF3, h2o, of2?​

Answer 1

Answer:

dffggtTgttr1execrcrfyv5g6h

Answer 2

Bond angle & Electronegativity:

Explanation:

• The bond angle is inversely proportional to the electronegativity of the compound. A more electronegative compound pulls the electrons towards itself thus decreasing the charge density at the central atom. This results in decreasing bond angle.

• The NH3 molecular has trigonal pyramidal geometry. In NH3, N-H has a bond angle of 101.7° & H-H has a bond angle 107.8°  because the hydrogen atoms are repelled by the lone pair of electrons on the nitrogen atom. So the electronegativity of nitrogen is 3.04 and of hydrogen is 2.2. So the electronegativity of a molecule is 0.84.

• In NF3, the central nitrogen atom has four electron groups surrounding it. Out of which three are single bonds and one is lone pair. Therefore, it has tetrahedral geometry. The bond angle between F-F is 102.50° while a bond angle between N-F is 102°. As a result, the electronegativity of fluorine is 3.98 and nitrogen is 3.04. So the electronegativity of a molecule is 0.94.

• An oxygen atom has 6 electrons out of which two of them are bonded with a hydrogen atom leaving two lone pairs of electrons. Due to the presence of these lone pairs of electrons in H2O, the bond angle is 104.50°, resulting a molecule in a tetrahedral shape. Hydrogen has an electronegativity 2 while oxygen has an electronegativity of 3.5. So the electronegativity of a molecule is 1.4